Use the standard half-cell potentials listed below to calculate the standard cel

Question

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 degree C. (The equation is balanced.) 3 Cl_2 + 2 Fe rightarrow 6 Cl^-(aq) + 2 Fe^3+(aq) Cl_2 + 2 e^- rightarrow 2 Cl^-(aq) E degree = +1.36 V Fe^3+(aq) + 3 e^- rightarrow Fe E degree = -0.04 V +4.16 V -1.40 V -1.32 V +1.32 V + 1.40 V Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 degree C. (The equation is balanced.) Mg(s) + Cu^2+ (aq) rightarrow Cu(s) + Mg^2+ (aq) Mg^2+ (aq) + 2e^- rightarrow Mg(s) E degree = -2.38 V Cu^2+ (aq) + 2e^- rightarrow Cu(s) E degree = +0.34 V +2.04 V -2.04 V +2.72 V -1.36 V +1.36 V

Explanation / Answer

19)

we know that

oxidation takes place at anode

and

reduction takes place at cathode

soo

anode : oxidation

Fe ---> Fe+3 + 3e-

cathode : reduction

Cl2 + 2e- ---> 2Cl-

now

we know that

Eo cell = Eo cathode - Eo anode

so

Eo cell = Eo Cl2 / 2Cl- - Eo Fe+3 / Fe

Eo cell = 1.36 - ( -0.04)

Eo cell = 1.40

so

the answer is option E) 1.40 V

20)

anode : oxidation

Mg ---> Mg+2 + 2e-

cathode : reduction

Cu+2 + 2e- ---> Cu

now

Eo cell = Eo cathode - Eo anode

so

Eo cell = Eo Cu+2 /Cu - Eo Mg+2 / Mg

Eo cell = 0.34 - (-2.38)

Eo cell = 2.72 V

so

the answer is C) 2.72 V

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